The equilibrium constants for the reactions X | vedclass

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(A) Let the initial concentration of $X$ and $Z$ be $C$ and $\alpha$ be the degree of dissociation.For reaction $X \rightleftharpoons 2Y$:Initial conc

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$4$

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(A) Let the initial concentration of $X$ and $Z$ be $C$ and $\alpha$ be the degree of dissociation.For reaction $X \rightleftharpoons 2Y$:Initial concentration: $C$ $0$Equilibrium concentration: $C(1-\alpha)$ $2C\alpha$$K_{1} = \frac{[2C\alpha]^2}{C(1-\alpha)} = \frac{4C^2\alpha^2}{C(1-\alpha)} = \frac{4C\alpha^2}{1-\alpha}$For reaction $Z \rightleftharpoons P + Q$:Initial concentration: $C$ $0$ $0$Equilibrium concentration: $C(1-\alpha)$ $C\alpha$ $C\alpha$$K_{2} = \frac{[C\alpha][C\alpha]}{C(1-\alpha)} = \frac{C^2\alpha^2}{C(1-\alpha)} = \frac{C\alpha^2}{1-\alpha}$Therefore,the ratio $\frac{K_{1}}{K_{2}} = \frac{4C\alpha^2 / (1-\alpha)}{C\alpha^2 / (1-\alpha)} = 4$.

The equilibrium constants for the reactions $X \rightleftharpoons 2Y$ and $Z \rightleftharpoons P + Q$ are $K_{1}$ and $K_{2}$,respectively. If the initial concentrations and the degree of dissociation of $X$ and $Z$ are the same,the ratio $K_{1} / K_{2}$ is

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